![13. Consider the reaction: 3 A(g) + B(gC (s) + 2D (g). The reaction was initiated with 0.50 mol A, 0.40 mol B and 0.20 mol D in a 1-L vessel. At equilibrium the [B] 0.30 M. What is the value of [D] at equilibrium?](http://img.homeworklib.com/questions/d9e34200-8c2e-11eb-ae56-21667d53f35c.png?x-oss-process=image/resize,w_560)
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13. Consider the reaction: 3 A(g) + B(gC (s) + 2D (g). The reaction was initiated...
show work please 3. Consider the following reaction where Kc 1.18 at 150K: 2HI(E)H2(g)+ 12(s) A...
show work please
3. Consider the following reaction where Kc 1.18 at 150K: 2HI(E)H2(g)+ 12(s) A reaction mixture was found to contain 0.0381 moles of HI, 0.0471 moles of H2, and 0.0364 moles of lz in a 1.00 L container. Is the reaction at equilibrium? And if not, what direction must it run in order to reach equiltibriurn? At equilibrium a 1.0-liter container was found to contain 0.20 mol of A, 0.20 mol of B, 0.40 mol of C, and...
3. Nitric oxide, NO(g) reacts with chlorine gas, Cl2(g), in the reaction 2NO(g) + Cl2(g) →...
3. Nitric oxide, NO(g) reacts with chlorine gas, Cl2(g), in the reaction 2NO(g) + Cl2(g) → 2NOCIG) Initial rates of reaction are determined for various combinations of initial concentrations of reactants and recorded below; Trial Initial [NO] (mol/L) 0.10 0.10 0.20 Initial (C12] (mol/L) 0.10 0.20 0.20 Rate of production of NOCI (mol/L.s) 1.8 x 107 3.6 x 102 1.43 x 10" a) What is the rate law equation for the reaction? (1 mark) b) What is the rate-determining step?...
6. Consider the reaction X + Y → Z Initial Rate of Disappearance of X (M/s)...
6. Consider the reaction X + Y → Z Initial Rate of Disappearance of X (M/s) [X] (M) [Y] (M) 0.053 0.10 0.50 0.127 0.20 0.30 1.02 0.40 0.60 0.254 0.20 0.60 0.509 0.40 0.30 From the data in the table, obtained at 360 K, (a) determine the overall order of the reaction (b) determine the initial rate of disappearance of X when the concentration of X is 0.30 M and that of Y is 0.40 M. ________ M/s
For the reaction 2A(g) + B(s) ⇌ C(l) + 2D(g) at 700 °C, Kc = 0.00147....
For the reaction 2A(g) + B(s) ⇌ C(l) + 2D(g) at 700 °C, Kc = 0.00147. Calculate the number of moles of D present at equilibrium if a mixture of 1.77 moles of C and 1.77 moles of D is heated to 700 °C in a 5.52-L container. The answer is 0.0650 mol but not sure how to get it.
For the reaction: 2 A (g) + B (s) ⇌ 2 C (s) + D (g)...
For the reaction: 2 A (g) + B (s) ⇌ 2 C (s) + D (g) Kp = 8210 At 298 K in a 10.0 L vessel, the known equilibrium values are as follows: 0.087 atm of A, 0.22 mol of B, and 10.5 mol of C. What is the equilibrium partial pressure of D?
Ch. 13 NAME 1. Consider the reaction: 2NO (g)+ 2H:(g) N2(g)+ 2H O (g) At a...
Ch. 13 NAME 1. Consider the reaction: 2NO (g)+ 2H:(g) N2(g)+ 2H O (g) At a certain temperature, the equilibrium concentrations are [NO]-0.31 M [H2]-0.16 M [N2] 0.082 M and [H:0]-4.64 M (a) Write the equilibrium expression for the reaction. (b) Determine the value of the equilibrium constant 2. The equilibrium constant Kc for the following reaction is 150.7 at 1 15°C: 12 (g) + Br2 (g) ←→ 2 IBr(g) 2.00 moles of each gas (l2, Br: and IBr) are...
3. Consider the decomposition reaction: 5A (g) 근 2 B(g) + C(g). You place 3.00 mol of A(g) in a reaction vessel mainta...
3. Consider the decomposition reaction: 5A (g) 근 2 B(g) + C(g). You place 3.00 mol of A(g) in a reaction vessel maintained at P-2 bar and T-298.15 K. For this reaction, ΔGor-70.0 kJ/mol (a) Derive an exact expression for Kpin terms of the extent of reaction at equilibrium, ξeq (b) Calcaulate the value licatons you make.
3. Consider the decomposition reaction: 5A (g) 근 2 B(g) + C(g). You place 3.00 mol of A(g) in a reaction vessel maintained...
23. The rate constant for a particular reaction is 27 activation energy for the reaction in...
23. The rate constant for a particular reaction is 27 activation energy for the reaction in kj/mol (R at 75 lut 25°C and 6 8.314 J/ mol.K) What is the 24. Initial rate data were obtained for the following reaction: A(g) + 2B(g) C + D(e) initial initial TA, mol/l. [B], molt initial rite Experiment 0.45 0.15 0.30 0.15 0.10 0.10 0.20 1.8 0.9 What are the rate law and k value for the reaction? 25. A mixture of 0.100...
Consider the equilibrium C(s)+ CO2(g) ⇌2 CO(g) A 2.0 L flask contains a mixture of 0.10...
Consider the equilibrium C(s)+ CO2(g) ⇌2 CO(g) A 2.0 L flask contains a mixture of 0.10 mol of CO(g), 0.20 mol of CO2(g) and 0.40 mol of C(s) in equilibrium at 700°C. *Note that only atm pressure values are allowed in the K expression.* The value of the equilibrium constant K is
For an equilibrium reaction at a particular temperature, 2 A+B=20 a) One equilibrium mixture has the...
For an equilibrium reaction at a particular temperature, 2 A+B=20 a) One equilibrium mixture has the following concentrations: [A] = 0.30 M, [B] - 0.20 M, and [C] = 0.50 M. Calculate the value of K. b) Another reaction mixture has the following concentrations: [A] = 0.40 M, [B] = 0.40 M, [C] = 0.40 M. Is this mixture at equilibrium? If not which direction will the reaction move to reach equilibrium?
show work please
3. Consider the following reaction where Kc 1.18 at 150K: 2HI(E)H2(g)+ 12(s) A reaction mixture was found to contain 0.0381 moles of HI, 0.0471 moles of H2, and 0.0364 moles of lz in a 1.00 L container. Is the reaction at equilibrium? And if not, what direction must it run in order to reach equiltibriurn? At equilibrium a 1.0-liter container was found to contain 0.20 mol of A, 0.20 mol of B, 0.40 mol of C, and...
3. Nitric oxide, NO(g) reacts with chlorine gas, Cl2(g), in the reaction 2NO(g) + Cl2(g) → 2NOCIG) Initial rates of reaction are determined for various combinations of initial concentrations of reactants and recorded below; Trial Initial [NO] (mol/L) 0.10 0.10 0.20 Initial (C12] (mol/L) 0.10 0.20 0.20 Rate of production of NOCI (mol/L.s) 1.8 x 107 3.6 x 102 1.43 x 10" a) What is the rate law equation for the reaction? (1 mark) b) What is the rate-determining step?...
Ch. 13 NAME 1. Consider the reaction: 2NO (g)+ 2H:(g) N2(g)+ 2H O (g) At a certain temperature, the equilibrium concentrations are [NO]-0.31 M [H2]-0.16 M [N2] 0.082 M and [H:0]-4.64 M (a) Write the equilibrium expression for the reaction. (b) Determine the value of the equilibrium constant 2. The equilibrium constant Kc for the following reaction is 150.7 at 1 15°C: 12 (g) + Br2 (g) ←→ 2 IBr(g) 2.00 moles of each gas (l2, Br: and IBr) are...
3. Consider the decomposition reaction: 5A (g) 근 2 B(g) + C(g). You place 3.00 mol of A(g) in a reaction vessel maintained at P-2 bar and T-298.15 K. For this reaction, ΔGor-70.0 kJ/mol (a) Derive an exact expression for Kpin terms of the extent of reaction at equilibrium, ξeq (b) Calcaulate the value licatons you make.
3. Consider the decomposition reaction: 5A (g) 근 2 B(g) + C(g). You place 3.00 mol of A(g) in a reaction vessel maintained...
23. The rate constant for a particular reaction is 27 activation energy for the reaction in kj/mol (R at 75 lut 25°C and 6 8.314 J/ mol.K) What is the 24. Initial rate data were obtained for the following reaction: A(g) + 2B(g) C + D(e) initial initial TA, mol/l. [B], molt initial rite Experiment 0.45 0.15 0.30 0.15 0.10 0.10 0.20 1.8 0.9 What are the rate law and k value for the reaction? 25. A mixture of 0.100...
For an equilibrium reaction at a particular temperature, 2 A+B=20 a) One equilibrium mixture has the following concentrations: [A] = 0.30 M, [B] - 0.20 M, and [C] = 0.50 M. Calculate the value of K. b) Another reaction mixture has the following concentrations: [A] = 0.40 M, [B] = 0.40 M, [C] = 0.40 M. Is this mixture at equilibrium? If not which direction will the reaction move to reach equilibrium?
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